5.1 Multiple-Choice and Bimodal Questions
1) Calculate the kinetic energy in J of an electron moving at 66.0010 m /s ?. The mass of an electron is 289.1110 g -?.
A) 484.9810-? B) 143.2810-? C) 171.6410-? D) 482.4910-? E) 146.5610-?
Answer: C Diff: 2
Page Ref: Sec. 5.1
2) Calculate the kinetic energy in joules of an automobile weighing 2135 lb and traveling at 55 mph. (1 mile = 1.6093 km, 1lb = 453.59 g).
A) 41.210? B) 52.910? C) 55.910? D) 63.210? E) 63.210-?
Answer: B Diff: 3
Page Ref: Sec. 5.1
3) The kinetic energy of a 7.3 kg steel ball traveling at 18.0 m/s is __________ J.
A) 3
?
1.210
B) 66
C) 3
?
2.410
D) 2
?
1.310
E) 7.3
Answer: A
Diff: 2
Page Ref: Sec. 5.1
4) Calculate the kinetic energy in joules of a 150 lb jogger (68.1 kg) traveling at 12.0 mile/hr (5.36 m/s).
A) 3
?
1.9610
B) 365
C) 978
D) 183
E) 68.1
Answer: C
Diff: 2
Page Ref: Sec. 5.1
5) Calculate the kinetic energy in joules of an 80.0 g bullet traveling at 300.0 m/s.
A) 6
?
3.6010
B) 4
1.2010
?
C) 3
?
3.6010
D) 12.0
E) 80.0
Answer: C
Diff: 2
Page Ref: Sec. 5.1
6) The kinetic energy of a 23.2-g object moving at a speed of 81.9 m/s is __________ J.
A) 145
B) 0.95
C) 77.8
D) 77,800
E) 1900
Answer: C
Diff: 2
Page Ref: Sec. 5.1
7) The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is __________ J.
A) 1900
B) 77.8
C) 145
D) 3
?
1.4310-
E) 6.00
Answer: E
Diff: 3
Page Ref: Sec. 5.1
8) The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is __________ kcal.
A) 3
?
1.4310-
B) 6.00
C) 1900
D) 454
E) 0.0251
Answer: A
Diff: 3
Page Ref: Sec. 5.1
9) A 100-watt electric incandescent light bulb consumes __________ J of energy in 24 hours. [1 Watt (W) = 1 J/sec]
A) 3
?
2.4010
B) 3
?
8.6410
C) 4.17
D) 3
?
2.1010
E) 6
?
8.6410
Answer: E
Diff: 3
Page Ref: Sec. 5.1
10) The ΔE of a system that releases 12.4 J of heat and does 4.2 J of work on the surroundings is __________ J.
A) 16.6
B) 12.4
C) 4.2
D) -16.6
E) -8.2
Answer: D
Diff: 2
Page Ref: Sec. 5.2
11) The value of ΔE for a system that performs 213 k J of work on its surroundings and loses 79 kJ of heat is __________ kJ.
A) +292
B) -292
C) +134
D) -134
E) -213
Answer: B
Diff: 2
Page Ref: Sec. 5.2
12) Calculate the value of ΔE in joules for a system that loses 50 J of heat and has 150 J of work performed on it by the surroundings.
A) 50
B) 100
C) -100
D) -200
E) +200
Answer: B
Diff: 2
Page Ref: Sec. 5.2
13) The change in the internal energy of a system that absorbs 2,500 J of heat and that does 7,655 J of work on the surroundings is __________ J.
A) 10,155
B) 5,155
C) -5,155
D) -10,155
E) 7
1.9110
?
Answer: C
Diff: 2
Page Ref: Sec. 5.2
14) The change in the internal energy of a system that releases 2,500 J of heat and that does 7,655 J of work on the surroundings is __________ J.
A) -10,155
B) -5,155
C) 7
-?
1.9110
D) 10,155
E) 5,155
Answer: A
Diff: 2
Page Ref: Sec. 5.2
15) The value of H ?? for the reaction below is -72 kJ. __________ kJ of heat are released when 1.0 mol of HBr is formed in this reaction.
22H (g)Br (g)2HBr(g)+→
A) 144 B) 72 C) 0.44 D) 36 E) -72
Answer: D Diff: 2
Page Ref: Sec. 5.4
16) The value of H ?? for the reaction below is -126 kJ. __________ kj are released when 2.00 mol of NaOH is formed in the reaction?
22222Na O (s)2H O(l)4NaOH(s)O (g)+→+
A) 252 B) 63 C) 3.9 D) 7.8 E) -126
Answer: B Diff: 2
Page Ref: Sec. 5.4
released by the reaction of 25.0 g of 22N a O with water is __________ kJ.
22222Na O (s)2H O(l)4NaOH(s)O (g)+→+
A) 20.2 B) 40.4 C) 67.5 D) 80.8 E) -126
Answer: A Diff: 3
Page Ref: Sec. 5.4
18) The value of H ?? for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is __________ kJ.
232S(s)?O (g)2SO (g)+→
A) 23 B) -23 C) -12 D) 12 E) -790
Answer: C Diff: 3
Page Ref: Sec. 5.4
released in the combustion of 16.0 g of 66C H (l)?
662222C H (l)?5O (g)12CO (g)6H O(l)+→+
A) 31.3410? B) 45.2310? C) 669
D) 32.6810? E) -6535
Answer: C Diff: 3
Page Ref: Sec. 5.4
20) The value of H ?? for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO (g) reacts completely.
222C O (g)燨(g)2C O (g)+→
A) 32.8910? B) 207 C) 103 D) 65.7 E) -482
Answer: C Diff: 3
Page Ref: Sec. 5.4
21) The value of H ?? for the reaction below is -336 kJ. Calculate the heat (kJ) released to the surroundings when 23.0 g of HCl is formed.
423C H (g)?C l (g)C H C l (l)3H C l(g)+→+
A) 177
B) 32.5710? C) 70.7 D) 211 E) -336
Answer: C Diff: 3
Page Ref: Sec. 5.4
22) The value of H ?? for the reaction below is -186 kJ. Calculate the heat (kJ) released from the reaction of 25 g of 2C l .
22 H (g)C l 2H C l(g)+→
A) 66
B) 25.3 ?10 C) 33 D) 47 E) -186
Answer: A Diff: 3
Page Ref: Sec. 5.4
23) The enthalpy change for the following reaction is -483.6 kJ:
2222H (g)O (g)2H O(g)+→
Therefore, the enthalpy change for the following reaction is __________ kJ:
2224H (g)2O (g)4H O (g)+→
A) -483.6 B) -967.2 C) 52.3410? D) 483.6 E) 967.2
Answer: B Diff: 2
Page Ref: Sec. 5.4
24) The value of H ?? for the reaction below is +128.1 kJ:
32C H O H (l)C O (g)2H (g)→+
How many kJ of heat are consumed when 15.5 g of 3C H O H (l) decomposes as shown in the equation?
A) 0.48 B) 62.0 C) 21.310? D) 32 E) 8.3
Answer: B Diff: 3
Page Ref: Sec. 5.4
32C H O H (l)C O (g)2H (g)→+
How many kJ of heat are consumed when 5.10 g of 2H (g) is formed as shown in the equation?
A) 162 B) 62.0 C) 128 D) 653 E) 326
Answer: A Diff: 3
Page Ref: Sec. 5.4
26) The value of H ?? for the reaction below is +128.1 kJ:
32C H O H (l)C O (g)2H (g)→+
How many kJ of heat are consumed when 5.10 g of CO(g)is formed as shown in the equation?
A) 0.182 B) 162 C) 8.31 D) 23.3 E) 62.0
Answer: D Diff: 3
Page Ref: Sec. 5.4
32C H O H (l)C O (g)2H (g)→+
How many kJ of heat are consumed when 5.75 g of CO(g) is formed as shown in the equation?
A) 23.3 B) 62.0 C) 26.3 D) 162 E) 8.3
Answer: C Diff: 3
Page Ref: Sec. 5.4
28) The value of H ?? for the reaction below is -1107 kJ:
22Ba(s)O (g)2BaO (s)+→
How many kJ of heat are released when 5.75 g of Ba(s) reacts completely with oxygen to form BaO(s)?
A) 96.3 B) 26.3 C) 46.4 D) 23.2 E) 193
Answer: D Diff: 3
Page Ref: Sec. 5.4
22Ba(s)O (g)2BaO (s)
+→
How many kJ of heat are released when 5.75 g of BaO(s) is produced?
A) 56.9 B) 23.2 C) 20.8 D) 193 E) 96.3
Answer: C Diff: 3
Page Ref: Sec. 5.4
30) The value of H ??for the reaction below is -1107 kJ:
22Ba(s)O (g)2BaO (s)+→
How many kJ of heat are released when 15.75 g of Ba(s) reacts completely with oxygen to form BaO(s)?
A) 20.8 B) 63.5 C) 114 D) 70.3 E) 35.1
Answer: B Diff: 3
Page Ref: Sec. 5.4
31) The molar heat capacity of a compound with the formula
C H SO is 88.0 J/mol-K.
26
The specific heat of this substance is __________ J/g-K.
A) 88.0
B) 1.13
C) 4.89
D) 3
?
6.8810
E) -88.0
Answer: B
Diff: 3
Page Ref: Sec. 5.5
32) A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample increases from 23.2 °C to 30.5 °C. Since the specific heat capacity of aluminum is
0.90 J/g-K, the mass of the sample is __________ g.
A) 72
B) 1.5
C) 65
D) 8.1
E) 6.6
Answer: B
Diff: 3
Page Ref: Sec. 5.5
33) The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15g of lead from 22 °C to 37 °C?
A) 2.0
B) -0.13
C) 4
5.8 ?0-
D) 29
E) 0.13
Answer: D
Diff: 3
Page Ref: Sec. 5.5
34) The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0 J of heat. The specific heat capacity of the lead is __________ J/g-K.
A) 7.8
B) 1.9
C) 29
D) 0.13
E) -29
Answer: D
Diff: 3
Page Ref: Sec. 5.5
35) The specific heat of bromine liquid is 0.226 J/g · K. The molar heat capacity (in
J/mol-K) of bromine liquid is __________.
A) 707
B) 36.1
C) 18.1
D) 9.05
E) 0.226
Answer: B
Diff: 3
Page Ref: Sec. 5.5
36) The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to raise the temperature of 10.0 mL of bromine from 25.00 °C to 27.30 °C? The density of liquid bromine: 3.12 g/mL.
A) 5.20
B) 16.2
C) 300
D) 32.4
E) 10.4
Answer: B
Diff: 4
Page Ref: Sec. 5.5
37) The ΔH for the solution process when solid sodium hydroxide dissolves in water is 44.4 kJ/mol. When a 13.9-g sample of NaOH dissolves in 250.0 g of water in a coffee-cup calorimeter, the temperature increases from 23.0 °C to __________ °C. Assume that the solution has the same specific heat as liquid water, i.e., 4.18 J/g-K.
A) 35.2 °C B) 24.0 °C C) 37.8 °C D) 37.0 °C E) 40.2 °C
Answer: D Diff: 4
Page Ref: Sec. 5.5
38) ΔH for the reaction
532IF (g) IF (g)F (g)→+ is __________ kJ, give the data below.
23IF(g)F (g) IF (g)+→ ΔH = -390 kJ
25IF(g)2F (g) IF (g)+→ ΔH = -745 kJ
A) +355 B) -1135 C) +1135 D) +35 E) -35
Answer: A Diff: 3
Page Ref: Sec. 5.6
232Fe O (s)3C O (s)2Fe(s)3C O (g)+→+ ΔH = -28.0 kJ 22343Fe(s)4C O (s)4C O (g)Fe O (s)+→+ ΔH = +12.5 kJ
the enthalpy of the reaction of 23Fe O with CO 232343Fe O (s)CO (g)CO (g)2Fe O (s)+→+ is __________ kJ.
A) -59.0 B) 40.5 C) -15.5 D) -109 E) +109
Answer: A Diff: 3
Page Ref: Sec. 5.6
40) Given the following reactions
222N (g)2O (g)2N O (g)+→ ΔH = 66.4 kJ
222NO(g)O (g)2NO (g)+→ ΔH = -114.2 kJ
the enthalpy of the reaction of the nitrogen to produce nitric oxide
22N (g)O (g)2NO(g)+→
is __________ kJ.
A) 180.6 B) -47.8 C) 47.8 D) 90.3 E) -180.6
Answer: A Diff: 3
Page Ref: Sec. 5.6
(1) 222N O N O →+ ΔH = -180 kJ (2) 222N O O 2N O +→ ΔH = -112 kJ
the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide 222N 2O 2N O +→
is __________ kJ.
A) 68 B) -68 C) -292 D) 292 E) -146
Answer: A Diff: 3
Page Ref: Sec. 5.6
42) Given the following reactions:
232S(s)3O (g)2SO (g)+→ ΔH = -790 kJ 22S(s)O (g)SO (g)+→ ΔH = -297 kJ
the enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide
2232SO (g)O (g)2SO (g)+→
is __________ kJ.
A) 196 B) -196 C) 1087 D) -1384 E) -543
Answer: B Diff: 3
Page Ref: Sec. 5.6
32C aC O (s)C aO (s) +C O (g)→ ΔH = 178.1 kJ 22C (s, graphite)O (g)C O (g)+→ ΔH = -393.5 kJ
the enthalpy of the reaction 32C aC O (s)C aO (s)C (s, graphite)O (g)→++
is __________ kJ.
A) 215.4 B) 571.6 C) -215.4 D) -571.6 E) 47.0110?
Answer: B Diff: 3
Page Ref: Sec. 5.6
44) Given the following reactions
22H O (l)H O (g)→ ΔH = 44.01 kJ
2222H (g)+O (g)2H O (g)→ ΔH = -483.64 kJ
the enthalpy for the decomposition of liquid water into gaseous hydrogen and oxygen
2222H O (l)2H (g)+O (g)→
is __________ kJ.
A) -395.62 B) -527.65 C) 439.63 D) 571.66 E) 527.65
Answer: D Diff: 3
Page Ref: Sec. 5.6
22N (g)O (g )2NO(g)+→
ΔH = +180.7 kJ
222N O (g)O (g )2N O (g)+→ ΔH = -113.1 kJ
the enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen 2222N O (g)N (g)2O (g )→+
is __________ kJ.
A) 67.6 B) -67.6 C) 293.8 D) -293.8 E) 45.5
Answer: B Diff: 3
Page Ref: Sec. 5.6
46) Given the following reactions
22N (g)O (g )2NO(g)+→ ΔH = +180.7 kJ 222N O (g)O (g )2N O (g)+→ ΔH = -113.1 kJ
the enthalpy of reaction for
224N O (g)2N O (g )N (g)→+
is __________ kJ.
A) 67.6 B) 45.5 C) -293.8 D) -45.5 E) 293.8
Answer: C Diff: 3
Page Ref: Sec. 5.6